Part D Application of Hess's Law a. Write in your experimentally-derived thermochemical equations. (1) (2) enthalpy values in the following Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g) Mg0(s) + 2 HCl(aq) → MgCl₂(aq) + H₂O(1) AH₁ = ΔΗ, = b. Use Hess's Law to get AH3 for reaction (3) from AH₁ and AH₂. (3) Mg(s) + H₂O(1)→➜ MgO(s) + H₂(g) AH3 = c. Now calculate AH3 from standard molar enthalpies of formation found in the thermodynamic tables in the appendix.
Part D Application of Hess's Law a. Write in your experimentally-derived thermochemical equations. (1) (2) enthalpy values in the following Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g) Mg0(s) + 2 HCl(aq) → MgCl₂(aq) + H₂O(1) AH₁ = ΔΗ, = b. Use Hess's Law to get AH3 for reaction (3) from AH₁ and AH₂. (3) Mg(s) + H₂O(1)→➜ MgO(s) + H₂(g) AH3 = c. Now calculate AH3 from standard molar enthalpies of formation found in the thermodynamic tables in the appendix.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter5: Thermochemistry
Section: Chapter Questions
Problem 44E: Although the gas used in an oxyacetylene torch (Figure 5.7) is essentially pure acetylene, the heat...
Related questions
Question
Please answer
Transcribed Image Text:Part D Application of Hess's Law
a. Write in your experimentally-derived
thermochemical equations.
(1)
(2)
enthalpy values in the following
ΔΗ,
=
ΔΗ, =
Mg(s) + 2 HCl(aq) → MgCl₂(aq) + H₂(g)
Mg0(s) + 2 HCl(aq) → MgCl₂(aq) + H₂O(1)
b. Use Hess's Law to get AH3 for reaction (3) from AH₁ and AH₂.
(3) Mg(s) + H₂O(1)→ MgO(s) + H₂(g)
AH3 =
c. Now calculate AH3 from standard molar enthalpies of formation found in the
thermodynamic tables in the appendix.
d. Discussion: Compare your experimental value of AH3 with the value calculated
from the thermodynamic tables. Can you explain why they shouldn't be exactly
the same?
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps with 2 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning